Le Chateliter\'s Principle. Determine in which direction the reaction will shift
ID: 895753 • Letter: L
Question
Le Chateliter's Principle. Determine in which direction the reaction will shift in each case . Assume the system intially is at equilibrium. A(g)+B2(g) 3C(g)+D(g) Pressure is increased. A(g)+B2(g) 3C(l)+D(g) Volume of vessel is doubled. A(g)+B(g) 3C(s)+D(g) Exothermic reaction, temperature .s increased. A(g),+B(g) 3C(s)+D(g) Endothermic reaction, catalyst is added. A(g)+Bj2(g) 3C(s)+D(g) Concentration of is tripled. A(g)+B2(g) 3C(g)+D(g) Amount of C is doubled. A(g)+B(g) 3C(g)+D(g) The endothermic gas reaction in a chamber is cooled. 0.250 moles of H2 and 0.250 moles of l2 were placed in a 1.00 I flask at 500degeee. The equilibrium constant, Kc for the reaction H2(g) + I2{g) 2HI (g) is 54.3. Calculate the equilibrium concentrations of all species.Explanation / Answer
13. The position of equilibrium moves to the right if you increase the pressure.
14. Doubling the volume, doubles the forward rate of reaction I.e.,position of equilibrium shifts towards right.
15. The position of equilibrium shifts to the left if you increase the temperature and exothermic.
16. The position of equilibrium shifts to the left if reaction is endothermic and catalyst have no effect on the position.
17. The position of equilibrium shifts to the right if the concentration of D is tripled.
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